One can calculate the molar solubility of a conic marble sample, predominantly made of CaCO3, when exposed to acid rain with a pH of 4.34 using the following information: CaCO3) + H2O) + CO2la0) = Ca2*aq) + 2 HCO, (aq) K = ? CaCO36) = Ca2"nq) + CO,2"(a) Kp = 2.8 x 10 CO2laq) + 2 H2O) = H3O°uq) + HCO3'cam) K1 - 4,4 x 107 HCO3 (an) + H2O) =H3O*taq) + CO,²'wa) K2 = 4.7 x 1011 2 H2Ou= H3Oʻsao) + OH'aol Kw- 1.0 x 1014 A water sample from around the marble is collected into a conical container. Assuming that the calcium is purely from the marble sample, and basing your calculations off of the molar solubility, calculate how many grams of calcium are present in this water sample. Note that the cone has a base radius of 10.00mm and a height of 480.8mm. molar solubility of CaCO3 = M amount of calcium= --× 103 g

One can calculate the molar solubility of a conic marble sample, predominantly made of CaCO3, when exposed to acid rain with a pH of 4.34 using the following information: CaCO3) + H2O) + CO2la0) = Ca2aq) + 2 HCO, (aq) K = ? CaCO36) = Ca2"nq) + CO,2"(a) Kp = 2.8 x 10 CO2laq) + 2 H2O) = H3O°uq) + HCO3'cam) K1 - 4,4 x 107 HCO3 (an) + H2O) =H3Otaq) + CO,²'wa) K2 = 4.7 x 1011 2 H2Ou= H3Oʻsao) + OH'aol Kw- 1.0 x 1014 A water sample from around the marble is collected into a conical container. Assuming that the calcium is purely from the marble sample, and basing your calculations off of the molar solubility, calculate how many grams of calcium are present in this water sample. Note that the cone has a base radius of 10.00mm and a height of 480.8mm. molar solubility of CaCO3 = M amount of calcium= --× 103 g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the solubility-product constant for each of the following substances, given that the molar concen- trations of their saturated solutions are as indicated: -8 (a) AgSeCN (2.0 × 10−8 M; products are Ag† and SeCN). -6 RaSO4 (6.6 × 10¯6 M). (b) (c) Pb(BrO3)2 (1.7 × 10¯¹ M). (d) Ce(IO3)3 (1.9 × 10-³ M). -3
A flask contains the following chemical system at equilibrium Ca(OH)2(s) f Ca2+(aq) + 2 OH - (aq) Addition of which of the following substances will increase the solubility of Ca(OH)2(S) A) NHO3(aq) B) Ca(OH)2(S) C) NaOH(S) D) CaCL2(s) E) Ca(NO3)2(s)
Solid cobalt(II) nitrate is slowly added to 50.0 mL of a 0.0541 M sodium hydroxide solution. The concentration of cobalt(II) ion required to just initiate precipitation is M. (Assume that Ksp (Co(OH)2)= 2.5 x 10^-16).
What is the molar solubility of calcium sulfate, CaSO4, at 25°C? The solubility product constant for calcium sulfate is 2.4  10–5at 25°C.A) 2.4  10–5 MB) 3.5  10–2 MC) 1.2  10–5 MD) 1.8  10–2 ME) 4.9  10–3 M
Complete the following solubility constant expression for Fe(OH)2. Kn 0 sp 010
The Solubility Product Constant for lead phosphate is 3.0 × 10-4. The molar solubility of lead phosphate in a 0.286 M ammonium phosphate solution is M.
The ?spKsp of lanthanum fluoride, LaF3LaF3 , is 2.00×10−192.00×10−19 . Calculate the molar solubility, ?s, of this compound.
Consider a mixture of 75.0 mL of 1.00 × 10−6 M thallium nitrate (TlNO3(aq)) and 100.0 mL of seawater (0.51 M in NaCl(aq)) (a) What sparingly soluble compound may form? Write out the chemical equation for its solubility equilibrium, its Ksp expression and the value of its Ksp. (b) Will a precipitate form from this mixture? Justify your answer.
What is the molar solubility of calcium oxalate, CaC2O4, in a 0.170 M calcium chloride solution? The solubility product constant for calcium oxalate is 2.3 x 10-9. Molar solubility =| M
What is the molar solubility of silver carbonate (Ag2CO3) in water? The solubility-product constant for Ag2CO3 is 8.1 x 10-12 at 25 °C.
The Ksp of magnesium carbonate, MgCO3, is 6.82 × 106. Calculate the molar solubility, S, of this compound. M S =
Solid silver acetate is slowly added to 50.0 mL of a 0.0620 M sodium sulfite solution. The concentration of silver ion required to just initiate precipitation is ? M. (Assume that Ksp (AgSO3)= 1.5 x 10^-14.)